required

the protons are not equal to the electrons ion the protons are not equal to the neutrons isotope atomic mass = mass of protons + neutrons changing the number of neutrons does not influece the mass or electrons atom behaviour is because of electrons hydrogen almost always loses its electron, leaving it a hydrogen ion taking away a negative charge creates a cation adding a negative charge creates an anion electronegativity is the ability to steal electrons electronegativity is influenced by the number of electrons needed to complete the valence shell nonpolar covalent bonds: electrons are shared equally polar bonds: electrons are shared unequally; pulled more toward one atom and have charge hydrogen bonds- when H forms a polar bond with another atom, it takes on a slightly positive charged and is attracted to any nearby negatively charged atoms acids = proton donators bases = proton acceptors ionic bonds: occur when valence electrons are transferred from one atom to another, and form ions solvent = the dissolving agent solute = the substance that is dissolved covalent bonds between C and H are non-polar neutrality is repelled by charge strong acids have a very high concentration of protons strong bases have a very high concentration of hydroxide buffers: molecules that slow down changes in pH by combining with or releasing H ions normal pH range in blood is 7.35-7.45 functional group: the stuff that hangs off carbon chain
O=C carbonyl
OH hydroxyl
SH sulfhydryl
NH2 amino
O=C-OH carboxyl
OH-O-P-OH-O phosphate condenstation reactions: covalent bond, builds a larger molecules from smaller ones, output is H2O hydrolysis reactions: ionic or covalent bond, splits larger molecules into smaller ones, breaks down water carbohydrates are made up of covalent bonds
1:2:1 ratio of C H and O monosaccharide example: ribose disaccharides are joined by condensation disaccharide example: lactose (glucose & galactose) and sucrose (glucose &